Objectives: 1. I can classify matter into substances and mixtures.

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1 Objectives: 1. I can classify matter into substances and mixtures.2. I can identify and distinguish between physical and chemical properties.3. I can identify and distinguish between the two types of forces that affect the nature of molecules.4. I can understand and distinguish between physical and chemical changes.5. I can identify techniques used to separate mixtures.

2 Daily Objective I can define matter.I can identify and distinguish between the classes of matter.2

9 Classification of MatterTerms: element, compound, mixture, substance, homogenous mixture, and heterogenous mixture.Define/illustrate each term above.2. Use a graphic organizer to show how these terms are connected to matter and each other.

23 Classifying Matter: Substances vs. MixturesElementPure and simplest substanceOne type of atomPeriodic tableSymbol, (He= Helium)Homogenous Mixture2 or more substances physically combined.Substances are very soluble in one another-mix well – one phaseSubstances in mix properties are preservedSeparated by physical processes.Also called a solutionEx. salt water, kool-aidCompound2 or more substances chemicallycombinedDefinite compositionBreak-down only thru chemical processesSubstances making up cmpd gain new properties.Chemical Formula, H2OEx. iron rustHeterogenous MixtureSubstances are not soluble in one another-do not mix well-multiple phasesSubstances in mixture properties are preserved.Separated by physical processesEx. Oil and water, pizza, soil

25 Exit Slip Classify the following examples two ways:Substance or Mixture?Element, Compound, Heterogenous mixture or Homogenous mixture?gasoline at the pumpsalt you garnish fries withaluminum foilsand

28 Classifying Matter represents an atomphysical combination of substancesmultiple phasesone phasechemical combination of substancessame composition from sample to sampleindividual properties are preserved when substances combinevaried composition from sample to sampleindividual properties are lost and new properties are gained when substances combinechemical formulasolutionatom’s symbolsubstances dissolve in one another.

32 Objectives: 1. I can classify matter into substances and mixtures.2. I can identify and distinguish between physical and chemical properties.3. I can identify and distinguish between the two types of forces that affect the nature of molecules.4. I can understand and distinguish between physical and chemical changes.5. I can identify techniques used to separate mixtures.

35 Classification of Matter LabMatter’sNameOne or more phases(parts)Abbreviation of matter(Symbol/Formula)# of substance(s)Element,Compound,Hetro Mix,Homo Mix1tap water2Deionizedwater

36 Classification of Matter Lab QuestionsMatter’sNameOne or more phases(parts)Abbreviation of matter(Symbol/Formula)# of substance(s)Element,Compound,Hetro Mix,Homo Mix123456.

37 Conclusion: Classification of Matter LabWhat was most beneficial about this lab?What was most challenging about this lab?How has this lab helped you make important connections and distinctions between the classes of matter?

38 Classifying Matter LabStudents with peers observe various samples of matter and classify them as an element, compound, homo mixture, or hetero mixture.

40 Classifying Matter1. Classify each as either an element, compound, homo mixture, or hetero mixturea. soilb. orange juice with no pulpc. copper wired. car gasoline (C8H18)2. What is the difference between a compound and a mixture?

41 Bell Ringer: Matter What is the difference between:substances and mixturescompounds and mixtures2. Classify each of the following examples:sugarsugar watergold ringIron rust (FeO)Italian dressing

44 Classifying Matter LabO2 = compoundWhy?Because the subscript number represents atoms that are chemically bonded.In this example, two atoms of oxygen are chemically bonded together.

45 Chemical vs. Physical ChangeChemical Change:Matter’s chemical make-up changes.New matter is produced with new propertiesEx. Iron Rust (FeO)Physical Change:Matter’s chemical make-up stays the same.Matter is the same, so most properties are the same.Ex. Lemonade

46 Intramolecular ForcesForces within a compound that holds the atomstogether. Also called chemical bonds.H2O compound

54 Mixture Separation LabStudents work in groups to determine what physical processes they can use to separate out each substance in a given mixture.They will design and carry out their experiment to successfully separate out each substance in the mixture.Reiterate the concept that substances in a mixture maintain their physical properties because their chemical make-up is preserved.

55 Mixture Separation Lab (9/11)Purpose: To design and carry-out an experiment that will separate substances from a mixture.

56 Homongenous Mixtures Also called solutions. Solutions:-Solute: what is dissolved-Solvent: what dissolves.

57 Solubility of MixturesSolubility: How well substances dissolvein one another.Chemistryland.comSciencephoto.com

58 Physical Separation of Mixtures: Extraction1. Extraction- separating substances in a heterogenous mixture from one another based on their unique physical properties..Physically separate oilfrom water becausethey are not soluble in one another.How could we separateiron fillings and sand?

59 Physical Separation of Mixtures: FiltrationCommonly used to separate a solid from a liquid in a heterogenous mixture due to differences in size or solubility.

60 Physical Separation of Mixtures DistillationSeparation of liquids in a mixture by their differences in boiling points. Ex. Ethanol (78 0C) and Water (1000C)

61 Chromotography Separates homogenous mixtures based on solubility.Chromotography has two phases:-Stationary Phase: solidMobile Phase: liquid or gasSubstances in mixture will separatebased on their degree of solubilitytoward the mobile phase.

67 Matter and Energy I can….Establish a relationship between changes in matter, the forces involved, and the flow of energy.

68 Bell Ringer1. Using your states of matter table what is the relationship between the following:intermolecular forces and kinetic energy?2. Complete the table below using the states of matter table and phases of matter diagramChanges in stateof matterKinetic Energy:Absorbed or ReleasedIntermolecular Forces:Strengthened orWeakenedevaporation of watercondensationof alcoholdeposition of coppermelting of ice cream

73 Heat Energy Heat Energy (q) =Energy that is transferred between matter of different temperatures.Unit for Energy: Joules (J) or calories (cal)1 J = calEnergy does not have mass or volume, therefore it is NOT classified as matter.How does heat energy flow between objects?Always flow from hot to cold objects73

74 Heat Energy Flow Heat energy flowing between objects: System:The matter you are studying/measuring.Surrounding :The matter (environment) around the system.Endothermic Process:When heat is absorbed by the system.Exothermic Process:When heat is released by the system.74

81 Conservation of Matter and EnergyMatter undergoeschanges, but the atoms are conserved as a whole or as parts.Energy:Energy is also conserved during changes that matter undergoes.If energy increases for a system, then its surroundings must decrease in energy by the same amount.81

82 Pre-APThe following slides pertain only to pre-AP chemistry classes.

83 Heat CapacityHeat Capacity: The amount of heat needed to raise the temperature of a substance 1.0 oC. What does heat capacity depend upon?

85 Specific Heat CapacitySpecific Heat Capcity: The amount of heat it takes to raise 1g of the substance 1 0C.

86 Heat CalculationThe temperature of a 95.4 g piece of copper increases from 25.0oC to 48.0oC when the copper absorbs 849 Joules of heat. What is the specific heat of copper?

87 Heat CalculationsHow much heat is required to raise the temperature of 250.0g of mercury to 52oC?

88 Bell RingerWhat is the difference between heat energy (q) and specific heat energy (C)?When J of energy is absorbed by a 42.1 g sample of silver the temperature increases by 15.0oC. What is the specific heat of silver?3. If an 8.8 gram sample of aluminum increases in temperature from 25oC to 55oC how much heat was absorbed by the aluminum sample?